Ayato and Itto would like to prepare 250 mL of 0.500 M phosphate buffer with pH 12.5. Here are some information about the solids: Relevant Reaction: Ka, = 7.5 x 10-3 H,PO4 Kaz = 6.2 x 10-8 Kaz = 4.8 x 10-13 %3D H3PO4 HPO4 PO 3. Some information about the solids: Solids Molar Mass, g/mol pure H3PO4 NaH2PO4-2H2O N22HPO4-2H2O NaзPO4:12H20 97.994 156.008 177.99, 380.132 1. Help them determine the following: a. Which appropriate solids should they use? b. Determine the amounts of the appropriate solids.

Ayato and Itto would like to prepare 250 mL of 0.500 M phosphate buffer with pH 12.5. Here are some information about the solids: Relevant Reaction: Ka, = 7.5 x 10-3 H,PO4 Kaz = 6.2 x 10-8 Kaz = 4.8 x 10-13 %3D H3PO4 HPO4 PO 3. Some information about the solids: Solids Molar Mass, g/mol pure H3PO4 NaH2PO4-2H2O N22HPO4-2H2O NaзPO4:12H20 97.994 156.008 177.99, 380.132 1. Help them determine the following: a. Which appropriate solids should they use? b. Determine the amounts of the appropriate solids.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question 7
True or False: NaBr can never be the salt of a buffer. http://www.sciencegeek.net/tables/ka.shtml O True O False
A buffer solution is made that is 0.337 M in H₂S and 0.337 M in KHS. If Kal for H₂S is 1.00 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.075 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) + +
Q3
One of the most common buffers used in protein chemistry is a weak base called TRIS (the nitrogen atom of the amino group is the basic portion of the molecule): Но. -NH2 (HOCH2);CNH, = TRIS %3D A biochemist prepares a buffer solution by adding enough TRIS and 12 M HCI to give 1.0 L of a buffer solution that has concentrations [TRIS] = 0.39 M and [TRISH*] = 0.56 M. (pK, of TRIS is 5.91.) (a) Calculate the pH of the buffer solution. pH = i (b) Suppose that 3.3 mL of 12 M HCI is added to 12 L of the buffer solution; calculate the new pH of the solution. pH = i
Determine the mass of solid NaCH,COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH;COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH,COOH is 1.8 x 10. NEXT > Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH;COOH(aq) + H2O(1) H,O (aq) CH;COO (aq) Initial (M) Change (M) Equilibrium (M)
What is the pH of the buffer solution that contains 1.0 g of NH₂Cl in 250 mL of 0.060 M NH,? Is the final pH lower or higher than the pH of the 0.060 M ammonia solution? ( Kb for ammonia is 1.8 × 10-5.) pH of the buffer= The final pH is solution. than the pH of the 0.060 M ammonia
Consider a solution that is 2.0×10-2 M in Fe²+ and 1.4x10-2 M in Mg²+. (Kap for FeCO3 is 3.07 x 10-¹1 and Kap for MgCO3 is 6.82 x 10-6) Show Transcribed Text If potassium carbonate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? O Fe²+ o Myột Show Transcribed Text What minimum concentration of K₂CO3 is required to cause the precipitation of the cation that precipitates first? Express your answer using two significant figures. 197| ΑΣΦ [K₂CO3] = Show Transcribed Tort ? M
2. A 0.15 M solution of HCI is saturated with H₂S. For H₂S (aq), Ka,1 = 8.9 x 10-8 and Ka,2 = 1.2 x 10-13. In a solution saturated with H₂S (g) at 1 atm, [H₂S (aq)] is 0.10 M. What is the concentration of S²-? What is the concentration of HS-? a. b.
7
(5e) Which two of the following compounds would you make a buffer of pH = 12.5. H3PO4 (MM=98.00 g/mol), NaH2PO4 (MM=119.98 g/mol), NazHPO4 (MM=141.96 g/mol), and Na3PO4 (MM = 163.94 g/mol)? [For H3PO4: pK; = 2.148; pKz=7.199; pK3=12.15]
A buffer solution with a pH of...